In the reaction NH4Cl = NH3 + HCl, the equilibrium concentrations were found to be [NH3] = [HCl]=3.71 * 10-3M
Calculate the value of the equilibrium constant?
K = (NH3)(HCl). Substitute and calculate K.
To calculate the value of the equilibrium constant (Kc) for the given reaction NH4Cl = NH3 + HCl, we can use the equation:
Kc = ([NH3] * [HCl]) / [NH4Cl]
Given that the equilibrium concentrations are [NH3] = [HCl] = 3.71 * 10^(-3) M, and assuming the initial concentration of NH4Cl to be zero, we have:
Kc = (3.71 * 10^(-3)M * 3.71 * 10^(-3)M) / 0
Since the initial concentration of NH4Cl is zero, the denominator is zero. Therefore, we cannot directly calculate Kc using this method.
However, we can use an alternative approach: the ratio of the equilibrium concentrations of the products to the reactants is equal to the equilibrium constant. Thus, we can write:
Kc = [NH3] * [HCl] / [NH4Cl]
Since the equilibrium concentrations of NH3 and HCl are equal (3.71 * 10^(-3)M), we can substitute these values into the equation:
Kc = (3.71 * 10^(-3)M * 3.71 * 10^(-3)M) / 3.71 * 10^(-3)M
Simplifying the equation:
Kc = (3.71 * 10^(-3)M) / 3.71 * 10^(-3)M
Kc = 1
Therefore, the value of the equilibrium constant (Kc) for the given reaction NH4Cl = NH3 + HCl is 1.